Iron oxide FeO crystallises in a cubic lattic | vedclass

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(D) The density formula for a unit cell is given by $d = \frac{Z 	imes M}{N_{A} 	imes a^3}$.Here,$d = 4.0 \ g \ cm^{-3}$,$M = 56 + 16 = 72 \ g \ mol

Vedclass · Accepted Answer

$4$

Vedclass · Answer

(D) The density formula for a unit cell is given by $d = \frac{Z 	imes M}{N_{A} 	imes a^3}$.Here,$d = 4.0 \ g \ cm^{-3}$,$M = 56 + 16 = 72 \ g \ mol^{-1}$,$a = 5.0 \ \mathring{A} = 5.0 	imes 10^{-8} \ cm$,and $N_{A} = 6.0 	imes 10^{23} \ mol^{-1}$.Substituting the values: $4.0 = \frac{Z 	imes 72}{6.0 	imes 10^{23} 	imes (5.0 	imes 10^{-8})^3}$.$4.0 = \frac{Z 	imes 72}{6.0 	imes 10^{23} 	imes 125 	imes 10^{-24}}$.$4.0 = \frac{Z 	imes 72}{0.075}$.$Z = \frac{4.0 	imes 0.075}{72} \approx 4.166$.The nearest integer value for the number of $FeO$ units per unit cell is $4$.

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